Question

Using the Table of Standard Reduction Potentials below, calculate the standard cell potential, E°cell, for the following redox reaction and determine whether this reaction is spontaneous as written under the standard conditions: E°cell = Is the reaction spontaneous? Cu(s) + Ni$^{2+}$(aq) ? Cu$^{2+}$(aq) + Ni(s). V. (Fill in the bank by entering the number with sign only. Report with 2 digits after the decimal point). (Fill in the blank by entering Yes or No only). Standard Reduction Potentials at 25 °C E° Reduction Half-Reaction (V) F$_2$(g) + 2 e$^-$ ? 2 F$^-$ (aq) 2.87 H$_2$O$_2$(aq) + 2 H$^+$ (aq) + 2 e$^-$ ? 2H$_2$O(l) 1.78 MnO$_4$$^-$(aq) + 8H$^+$ (aq) + 5 e$^-$ ? Mn$^{2+}$(aq) + 4 H$_2$O(l) 1.51 Cl$_2$(g) + 2 e$^-$ ? 2 Cl$^-$ (aq) 1.36 Cr$_2$O$_7$$^{2-}$(aq) + 14 H$^+$ (aq) + 6e$^-$ ? 2 Cr$^{3+}$(aq) + 7 H$_2$O(l) 1.33 O$_2$(g) + 4 H$^+$ (aq) + 4 e$^-$ ? 2 H$_2$O(l) 1.23 Br$_2$(l) + 2 e$^-$ ? 2 Br$^-$ (aq) 1.09 Ag$^+$ (aq) + e$^-$ ? Ag(s) 0.80 Fe$^{3+}$(aq) + e$^-$ ? Fe$^{2+}$(aq) 0.77 O$_2$(g) + 2 H$^+$ (aq) + 2e$^-$ ? H$_2$O$_2$(aq) 0.70 I$_2$(s) + 2 e$^-$ ? 2 I$^-$ (aq) 0.54 O$_2$(g) + 2 H$_2$O(l) + 4 e$^-$ ? 4 OH$^-$ (aq) 0.40 Cu$^{2+}$(aq) + 2 e$^-$ ? Cu(s) 0.34 Sn$^{4+}$(aq) + 2 e$^-$ ? Sn$^{2+}$(aq) 0.15 2 H$^+$ (aq) + 2 e$^-$ ? H$_2$(g) 0

          Using the Table of Standard Reduction Potentials below, calculate the standard cell potential, E°cell, for the following redox reaction
and determine whether this reaction is spontaneous as written under the standard conditions:
E°cell = 
Is the reaction spontaneous?
Cu(s) + Ni$^{2+}$(aq) ? Cu$^{2+}$(aq) + Ni(s).
V. (Fill in the bank by entering the number with sign only. Report with 2 digits after the decimal point).
(Fill in the blank by entering Yes or No only).
Standard Reduction Potentials at 25 °C
E°
Reduction Half-Reaction
(V)
F$_2$(g) + 2 e$^-$ ? 2 F$^-$ (aq)
2.87
H$_2$O$_2$(aq) + 2 H$^+$ (aq) + 2 e$^-$ ? 2H$_2$O(l)
1.78
MnO$_4$$^-$(aq) + 8H$^+$ (aq) + 5 e$^-$ ? Mn$^{2+}$(aq) + 4 H$_2$O(l)
1.51
Cl$_2$(g) + 2 e$^-$ ? 2 Cl$^-$ (aq)
1.36
Cr$_2$O$_7$$^{2-}$(aq) + 14 H$^+$ (aq) + 6e$^-$ ? 2 Cr$^{3+}$(aq) + 7 H$_2$O(l)
1.33
O$_2$(g) + 4 H$^+$ (aq) + 4 e$^-$ ? 2 H$_2$O(l)
1.23
Br$_2$(l) + 2 e$^-$ ? 2 Br$^-$ (aq)
1.09
Ag$^+$ (aq) + e$^-$ ? Ag(s)
0.80
Fe$^{3+}$(aq) + e$^-$ ? Fe$^{2+}$(aq)
0.77
O$_2$(g) + 2 H$^+$ (aq) + 2e$^-$ ? H$_2$O$_2$(aq)
0.70
I$_2$(s) + 2 e$^-$ ? 2 I$^-$ (aq)
0.54
O$_2$(g) + 2 H$_2$O(l) + 4 e$^-$ ? 4 OH$^-$ (aq)
0.40
Cu$^{2+}$(aq) + 2 e$^-$ ? Cu(s)
0.34
Sn$^{4+}$(aq) + 2 e$^-$ ? Sn$^{2+}$(aq)
0.15
2 H$^+$ (aq) + 2 e$^-$ ? H$_2$(g)
0

Using the Table of Standard Reduction Potentials below, calculate the standard cell potential, E°cell, for the following redox reaction
and determine whether this reaction is spontaneous as written under the standard conditions:
E°cell =
Is the reaction spontaneous?
Cu(s) + Ni^2+(aq) ? Cu^2+(aq) + Ni(s).
V. (Fill in the bank by entering the number with sign only. Report with 2 digits after the decimal point).
(Fill in the blank by entering Yes or No only).
Standard Reduction Potentials at 25 °C
E°
Reduction Half-Reaction
(V)
F2(g) + 2 e^- ? 2 F^- (aq)
2.87
H2O2(aq) + 2 H^+ (aq) + 2 e^- ? 2H2O(l)
1.78
MnO4^-(aq) + 8H^+ (aq) + 5 e^- ? Mn^2+(aq) + 4 H2O(l)
1.51
Cl2(g) + 2 e^- ? 2 Cl^- (aq)
1.36
Cr2O7^2-(aq) + 14 H^+ (aq) + 6e^- ? 2 Cr^3+(aq) + 7 H2O(l)
1.33
O2(g) + 4 H^+ (aq) + 4 e^- ? 2 H2O(l)
1.23
Br2(l) + 2 e^- ? 2 Br^- (aq)
1.09
Ag^+ (aq) + e^- ? Ag(s)
0.80
Fe^3+(aq) + e^- ? Fe^2+(aq)
0.77
O2(g) + 2 H^+ (aq) + 2e^- ? H2O2(aq)
0.70
I2(s) + 2 e^- ? 2 I^- (aq)
0.54
O2(g) + 2 H2O(l) + 4 e^- ? 4 OH^- (aq)
0.40
Cu^2+(aq) + 2 e^- ? Cu(s)
0.34
Sn^4+(aq) + 2 e^- ? Sn^2+(aq)
0.15
2 H^+ (aq) + 2 e^- ? H2(g)
0

Added by Barry F.

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